Solving for pH of a Buffer Solution, 3

Category: Chemical Engineering Math

"Published in Newark, California, USA"

What mass in grams of NaC₂H₃O₂ must be dissolved with 500 mL of 0.1 M acetic acid to make a buffer solution of pH = 5? K_a = 1.8 x 10^-5 for acetic acid.

Solution:

Buffer solution is a solution which is a mixture of weak acid and its salt or a mixture of weak base and its salt. The purpose of making a buffer solution is to prevent the rapid change of pH if acid or base is added to the solution. In this problem, the buffer solution is a mixture of acetic acid and sodium acetate. 

Let's consider the ionization of acetic acid as follows

The ionization constant for acetic acid is

If pH = 5 for the buffer solution, then the concentration of [H⁺] is

From the ionization of acetic acid, it follows that

Let's consider the ionization of sodium acetate as follows

If x is the concentration of sodium acetate, then it follows that

Again, let's consider the ionization constant of acetic acid as follows
 

 

If sodium acetate is added to acetic acid solution, then the concentration of acetate ion will increase as follows
 

 

Since 1 x 10^-5 is a very small number, then we can neglect it at the above equation as follows
 

 

 

Let's assume that the change of the volume of acetic acid is negligible if sodium acetate is added, then the volume of solution is also equal to 500 mL. 

Therefore, the weight of sodium acetate to be added with 500 mL of acetic acid is

Ionization Constant for Acid Problems, 5

Category: Chemical Engineering Math

"Published in Newark, California, USA"

When 0.02 moles of a monoprotic acid is dissolved in 350 mL of water, the pH is 3.05. What is the ionization constant of this acid?

Solution:

Monoprotic acid is an acid which donates one electron during the ionization process. Monoprotic acid can be an inorganic acid or organic acid as long as one electron is lost during the ionization process.

If the pH of an acid is 3.05, then the concentration of hydrogen ion is

Let's assume that the volume of water is equal to the volume of a solution because the amount of a monoprotic acid is very small or negligible. The concentration of a monoprotic acid at the start of ionization process is

Since the concentration of [H⁺] is very small compared with [HA], then HA is a weak acid. The ionization of HA is written as follows
 

Therefore, the ionization constant of a monoprotic acid is
 

 

 

 

Solving for pH of a Mixture of Acid and Base Problems

Category: Chemical Engineering Math

"Published in Newark, California, USA"

What is the pH of the resulting solution made by mixing 25 mL of 0.1 M HCl and 15 mL of 0.1 M NaOH?

Solution:

The given word problem is about the mixing of an acid and a base. If you mix an acid and a base, their products are salt and water. The chemical reaction for the given mixture is written as follows

In order to convert the HCl and NaOH completely into NaCl and water, you must have equal moles at each reactants which are HCl and NaOH. Let's see if the two reactants will be used completely as follows

Since the number of moles of HCl is greater than the number of moles of NaOH, then the resulting solution is an acid. 

Hence, the molarity of the resulting solution which is HCl is

              

Since HCl is a strong acid, then it is completely ionized as follows

Therefore, the pH of the resulting solution which is HCl solution is

 

Solving for pH of an Acid Problems, 2

Category: Chemical Engineering Math

"Published in Newark, California, USA"

Calculate the pH of 3.5 x 10^-3 M HNO₃.

Solution:

Let's consider the ionization of HNO₃ as follows 

Since HNO₃ is  a strong acid, then it is ionized completely into H⁺ and NO3^-. 

Therefore, the pH of a given solution is